Electrolysis:
- Electrolysis is a process in which an electric current is passed through a substance (usually a molten salt or an aqueous solution) to cause a chemical change.
- During electrolysis, the electrical energy causes the separation of ions into their elemental components.
- Electrolysis requires an external source of electrical energy to drive the chemical reaction.
- The products of electrolysis are typically two or more different substances.
Electrochemical Cells:
- Electrochemical cells, also known as galvanic cells or voltaic cells, are devices that convert chemical energy into electrical energy.
- In an electrochemical cell, a spontaneous chemical reaction occurs between two half-cells (oxidation and reduction half-reactions), generating an electric current.
- Electrochemical cells do not require an external power source; instead, they rely on the chemical reactions occurring within the cell to produce electricity.
- The products of an electrochemical cell are electricity and the reactants are consumed in the process.
To summarize, electrolysis uses electrical energy to drive chemical changes, while electrochemical cells convert chemical energy into electrical energy. Electrolysis requires an external power source, whereas electrochemical cells generate electricity through spontaneous chemical reactions.
